Interpretation:
The metal oxide that can be reduced to from metal on reaction with C atom from the given list needs to be determined using the coupled reactions method.
Concept introduction:
A non-spontaneous reaction can be changed to spontaneous reaction either by changing the reaction’s conditions like temperature or by combining the reaction with other reaction to get an overall spontaneous reaction. The spontaneity of the reaction can be determined with the help of sign of
At standard conditions, the
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- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardConsider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25Carrow_forwardTable 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.arrow_forward
- The ionization constant, Ka, for acetic acid is 1.8 105 at 25 C. What is the value of rG for this reaction? Is this reaction product- or reactant-favored at equilibrium?arrow_forwardUsing the given thermodynamic data in the table, determine the standard change in Gibbs free energy for this reaction at 298 K for the reaction of silver with hydrogen: 2Ag+(aq) + H2(g)2H+(aq) + 2Ag(s) Δ H f o / kJ∙mol –1 S o / J∙mol –1 ∙K –1 Ag + (aq) 105.58 72.68 Ag(s) 0 42.55 H 2 (g) 0 130.68 H + (aq) 0 0 Options: A. 48.7 kJ B. +162.5 kJ C. +268.1 kJ D. –154.3 kJarrow_forwardCalculate the change in the Gibbs energy for the reaction below, at 25.O °C 2 Ca(s) + O2(g) → 2 CaO(s) given ΔΗο, Prxn = -1269.8 kJ and ASºyn = -364.6 J/K. rxn O +470.5 kJ O +2355.9 kJ O -1161.1 kJ O -2352.8 kJarrow_forward
- The decomposition of a generic diatomic element in its standard state is represented by the equation X₂(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.71 kJ - mol-¹ at 2000. K and −55.51 kJ · mol-¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG₁ = 4.71 kJ · mol-¹. What is K at that temperature? K at 2000. K= At 3000. K, AGf = −55.51 kJ - mol-¹. What is K at that temperature? K at 3000. K =arrow_forwardThe solubility product constant, Ksp, at 25°C for AgI(s) in water has the value 8.3 × 10–17. Calculate ΔG at 25°C for the process AgI(s) ⟷⟷ Ag+(aq) + I–(aq) where [Ag+] = 9.1 × 10–9 M and [I–] = 9.1 × 10–9 M. (R = 8.314 J/K • mol)arrow_forwardThe decomposition of a generic diatomic element in its standard state is represented by the equation X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.13 kJ · mol-l at 2000. K and -61.50 kJ · mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG = 5.13 kJ · mol-1. What is K at that temperature? K at 2000. K = At 3000. K, AG¢ = -61.50 kJ · mol¬1. What is K at that temperature? K at 3000. K =arrow_forward
- NI3 decomposes as shown below: 2 Nl3(s) → N2(g) + 3 I2(g) Use the thermochemical information given below to calculate the standard Gibbs energy change (in kJ mol¬1) of this reaction at 298.15 K. NI3(s) N2(2) 2(g). AH;° (kJ mol-1) S° (J mol-1K-1) 287.0 62.40 230.0 191.6 260.7 O-161.1 O -387.0 O +513.7 +119.0 O -540.0arrow_forwardThe decomposition of a generic diatomic element in its standard state is represented by the equation x,(2) » X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.51 kJ · mol- at 2000. K and -57.84 kJ · mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG; = 5.51 kJ · mol-1. What is K at that temperature? K at 2000. K = At 3000. K, AG: = -57.84 kJ . mol-1. What is K at that temperature? K at 3000. K =arrow_forwardCalculate the standard Gibbs free energy changes at 25 °C for each of the reactions shown below using the Eº values given. Select whether each of these reactions is nonspontaneous, at equilibrium, or spontaneous under standard conditions. (a) 1 Cl₂(g) + 1 Mg(s) 2 Cl(aq) + 1 Mg2+ (aq) nonspontaneous at equilibrium O spontaneous Eº = 3.729 V AGO (b) 1 Ni2+ (aq) + 1 Ca(s) 1 Ni(s) + 1 Ca2+ (aq) E° = 2.590 V AG° = O nonspontaneous O at equilibrium spontaneous Submit Answer (c) 1 Ba2+ (aq) + 1 Hg(1) = 1 Ba(s) + 1 Hg2+ (aq) Eº = -3.754 V AG° = nonspontaneous at equilibrium spontaneous (d) 2 H+ (aq) + 1 Zn(s) = 1 H₂(g) + 1 Zn²+ (aq) Eº = 0.763 V AG⁰ O nonspontaneous O at equilibrium O spontaneous = Viewing Saved Work Revert to Last Response 11 kJ/mol kJ/mol kJ/mol kJ/molarrow_forward
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